CHEM 6A Study Guide - Quiz Guide: Nonmetal, Covalent Bond

Draw the lewis Dot Structure for the following molecules- You can use S=N-A or not. Remember a) get the best structure using the octet rule (assume all atoms have to obey the octet rule) b) determine the formal charge on each atom c) identify the elements which can have an expanded octet (row 3 and below) d) Try to reduce formal charges by redistributing electrons from elements on the periphery (usually these do not have more than 8 electrons) to the inner atoms which can accommodate expanded octets. e) make sure only atoms which can accommodate expanded octets actually have expanded octets. f) Make sure only atoms which are m groups 2, 3 have less than 8 electrons in their valence shell. O_3 PF_5 N_2O_4 5F_4 H_2CO_3 H_2CO H_2SO_3 SO_4^-2 BF_3 AlH_4^-1 CH_3CH_2NH_2 H_2O HF 2. Determine the electron domain geometry for each of the above compounds. Determine the molecular geometry for each of the compounds in question 1 Determine the hybridization for each of the atoms in question 1 Which of the compounds in question 1 will have a dipole? (first determine if polar covalent bonds exist, then see if they reinforce or cancel each other out) Which of the compounds in question 1 exhibit hydrogen bonding? Which of the compounds in question 1 exhibit resonance. Which of the compounds in question 1 exhibit dispersion forces? For the following organic molecules, determine the number of pi bonds, number of n bonds, number of sp^3, sp^2, sp hybridzed atoms, number of lone pairs, electronic domain geometries and molecular geometries.

Masteringchemistry Chaptery-hemical Bonding Lewis Theory- Gocgle Chrome 을 Secure ! https://session.masteringchemistry mView?offset-neyt&a 89499782 Covalent, Polar Covalent, and lonic Bonds Resources 《 previous | 80 1 Covalent, Polar Covalent, and lonic Bonds Part A Leaming Goal: Consider the following element combinations. Classify the bonds formed between each pair s ionic, polar covalent, or nonpolar covalent qualitatively based solely on each element's pasition on the periadic table Do not conduct calculations Drag the appropriate items to their respective bins. トHints To use electronegativity or metal versus nonmetal classifications to distinguish covalent, polar covalent, and ionic bonds When two bondod atoms attract electrons with equal strength, thec resull is a nonpolar covalet bond. A polacovalel bond is one in which the electrons are unequally shared between the atoms. An ionic hond resuits when the sharing is so unequal that fully charged ions form Eleclronegaivily difference an be used lo predict bond type. If electronegativities differ by more than 2 units, the bond is substantially ionic; if they difter by less than 2 units, the hond is polar covalent; and if the valucs arc cqual, the bond is nonpolar covalent. If you are ol given electronegativity values, you cari still predict the bond type using the perodic tabla. Metals havelow electronegativity compared to nonmetals So in general, we can predict that any metal- nonmctal combinaticn wil bc ionic and any nonmctal nonmetal combination wil be covalent. I「electronegativity values aren't given. you should assume that a covalent bond is polar unless it is behveen two atcoms of the same element Reset Help s and Br Cs and Cl B「and Br Ba and O O and Br P and i Mg and N P and F onic Polar covalent Submit My Answers Give Up Part B

First you need to find the number of valence electrons in NH_2Cl_2. For counting purposes with Lewis structures, the number of valence electrons in an atom of a main group element is equal to the last digit in the group number of that element in the Periodic Table. N is in Group __________ H is in Group _______________ Cl is in Group _____________ In NH_2Cl there is a total of ____________ valence electrons. The model consists of balls and sticks. How many holes should be in the ball you select for the N atom? __________ the H atoms? _____________ the Cl atom? ___________ The electrons in the molecule are paired, and each stick represents a valence electron pair. How many sticks do you need? ______________ Assemble a skeleton structure for the molecule, connecting the balls and sticks to make one unit. Use the rule that N atoms form three bonds, whereas Cl and H atoms usually form only one. Draw a sketch of the skeleton below: How many sticks did you need to make the skeleton structure? __________ How many sticks are left over? ____________ If your model is to be obey the octet rule, each ball must have four sticks in it (except for hydrogen atom balls, which need and can only have one). (Each atom in an octet rule species is surrounded by four pairs of electrons.) How many holes remain to be filled? _____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH_2Cl using lines for bonds and pairs of dots for nonbonding electrons. Describe the geometry of the model, which is that of NH_2Cl. __________ Is the NH_2Cl molecule polar? ___________ Why? Would you expect NH_2Cl to have any isomeric forms? _____________ Explain your reasoning. Would NH_2Cl have any resonance structures? __________ If so, draw them below.